(a) | Explain (b) Draw and describe the Cu-Zn electrochemical cell reactions. nme of C2H6 is Ethane? mole fra

Q: In a concentration cell, is the more concentrated electrolyte solution in the cathode or the anode…

A: Concentration cells are the cells with E0cell zero i.e the cathode and anode of the electrochemical…

Q: Calculate the number of grams of metal M produced in 1.055 hour by the electrolysis if the…

A:

Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: Given data Current (i) = 6 A Voltage (v) = 4.5 V Volume of K2Cr2O7 = 215 mL Concentration of K2Cr2O7…

Q: During a period of discharge of a lead–acid battery, 402 gof Pb from the anode is converted into…

A: Overall cell reaction is Pb(s) + PbO2(s) + 2H+ (aq) + 2HSO4- → 2 PbSO4 + 2H2O Where, 1 mol of Pb is…

Q: Elemental calcium is produced by the electrolysis of moltenCaCl2. (a) What mass of calcium can be…

A: a.

Q: A 0.15 M solution of KNO3 is electrolyzed at a voltage of 3.85 and a current of 1.18 amps for 12.0…

A:

Q: A current of 3.7A is passed for 6h between nickel electrodes in 0.5L of a 2M solution of Ni(NO3)2.…

A: We have to find the molarity

Q: Explain 3 applications of electrochemistry in common industrial processes and describe them in…

A: Electrochemistry is a branch of Chemistry in which different chemical changes take place by using…

Q: Write the net cell equation for this electrochemical cell. Phases are optional. Do not include the…

A: In this electrochemical cell of cobalt metal acts as a anode and silver metal is acts as a cathode.…

Q: Enter your answer in the provided box. Consider the following electrochemical cell in, for which E°…

A:

Q: If a water electrolysis cell operates at a current of 7.8 A, how longwill it take to generate 25.0 L…

A:

Q: (a) Based on standard reduction potentials, would youexpect copper metal to oxidize under standard…

A:

Q: During the discharge of an alkaline battery, 4.50 g of Znis consumed at the anode of the battery.…

A: Faraday's Law of Electrolysis: The Faraday's law of electrolysis states that the amount of electric…

Q: Metallic magnesium can be made by the electrolysis ofmolten MgCl2. (a) What mass of Mg is formed by…

A: (a) Mass formed by passing current can be given as: M: mass formed by metal on passing current.…

Q: Molten CaCl, can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

A:

Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: a) 215 ml  ofb1.25  potassium  means (1.25/1000)×215 = 0.26 mol of potassium dichromate.   From the…

Q: An electrolysis cell containing MSO4 solution is operated for 1.0 h at a constant current of 0.200…

A: Given,  An electrolysis of MSO4 solution for 1.0 h at a constant current of 0.200 A. If the current…

Q: What is the pH of the solution in the cathode half-cell inFigure when PH2 = 1.0 atm, [Zn2+] in the…

A: SOLUTION: Step 1: The anodic half-reaction and cathodic half-reaction that occurred in the…

Q: Crude copper containing Fe and Ag as contaminations was subjected toelectro refining by using a…

A: To find: the percentage of copper, iron and silver in crude copper.

Q: Agalvanie cell Za a" Ce"C costructed uning a completely immered Za electrode that weighs 31gand s Ce…

A:

Q: How long will it take to deposit 1.5 g of Cu on a metal when a current of 5 A is applied to a CuSO4…

A: Given- Amount of copper = 1.5 gMetal of interest = CuCurrent = 5 A To find- Time required

Q: A galvanic cell consists of Mg anode in a 1.0 M Mg(NO,), and Al cathode in a 1.0 M AI(NO,), solution…

A: The electrical energy can be calculated by using Nerst Equation

Q: It is desired to deposit 0.87 g of iron (MW = 55.85) from a FeCl3 solution by the passage of 2.5 A…

A: Given mass of of iron = 0.87 g MW for iron = 55.85 Current = 2.5 A Efficiency 85%

Q: How many moles of chromium would be electroplated by passing a current of 5.2 amperes through a…

A: Given, Current (I) = 5.2 A Time (t) = 45.0 min = (45.0 × 60) s = 2700 s Moles of chromium (Cr) = ?…

Q: (a) How many minutes does it take to form 10.0 L of O₂ measured at 99.8 kPa and 28°C from water if a…

A: Given- the volume of Oxygen(V) = 10 L = 0.01 m3     (Since 1 m3 = 1000 L) Temeperature(T)= 28 C…

Q: he table below gives the standard electrode potential values of some electrodes. A salt bridge is…

A: The electrochemical cells are made by connecting two electrodes of different potential. These cells…

Q: Calculate the minimum voltage in volts required to drive the electrolysis reaction of molten LiCl by…

A: The half-cell reactions are: Anode: Li(s) -----> Li+ + e- Eº = -3.03V Cathode: Cl2 + 2e-…

Q: 4. A commercial cell for producing F2 operates at a current of 1500A from the electrolysis of HF…

A:

Q: The potential of platinum versus saturated calomel electrode when polarized cathodically in…

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Q: A solution of a metal ion Mag is electrolyzed by a current of 5.00 A. After 10.0 minutes, 1.19 g of…

A: a.

Q: If the Standard Potential cell for the following AgI/Ag and I/I was -0.152vand o. Suv Pespectively.…

A:

Q: An electrode Is prepared fromm liquid mercury in contct willh a salurated solution o mercury(1)…

A: The standard reduction potentials of half- cell reactions are, The most positive standard reduction…

Q: Molten CaCl, can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

A: Given-> Current (I) = 2.99 ampere Weight of Ca= 23.5 gm

Q: Determining molar mass by electrolysis. An electrolysis cell containing MSO4 solution is operated…

A:

Q: A current of 8.46x1oʻ A is passed through an electrolysis cell containing molten KCi for 10.3 days.…

A: Given Current I = 8.46*104 A Time = 10.3 days Temperature = 273 K Pressure = 1 atm

Q: (a) Predict the products of electrolysis in each of the following:(i) An aqueous solution of AgNO3…

A: A voltaic cell is an example of electrochemical cell. It uses a chemical reaction to produce…

Q: The cell in Figure  could be used to provide a measureof the pH in the cathode half-cell. Calculate…

A: In the given cell, Cathode (Reduction half): 2H+(aq) + 2e- → H2(g)Anode (Oxidation half): Zn(s) →…

Q: Like any piece of apparatus, an electrolytic cell operates atless than 100% efficiency. A cell…

A: Current efficiency is the ratio of mass deposited to the theoretical mass deposited calculated by…

Q: (a)  What quantity of charge (in coulombs) is a fully      charged 12-V lead–acid storage battery…

A: Half reaction of the lead acid battey : Pb + SO42- —> PbSO4 + 2e- PbO2 + SO42- + 4H+ + 2e- —>…

Q: A solution of a metal ion ÷({ ) Q˘ is electrolyzed by a current of 5.00 A. After 10.0 minutes, 1.19…

A: Solution        1.a. Given that current,I=5.00A           time, t=10 minutes =10×60s…

Q: A solution containing a metal ion (M2+ (aq)) is electrolyzed by a current of 7.8 A. After 15.5…

A: The amount of substance that undergoes a chemical reaction at any electrode during electrolysis is…

Q: 6) Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below.…

A:

Q: In an electrolysis of a solution containing Ni2+ (aq), metallic Ni(s) deposits on the cathode. Using…

A: Given,  Current in ampere = I =  0.150 A  Electrolysis of Ni2+ (aq) ion  Time period in minutes = t…

Q: How long will it take to deposit 0.0047 mol of gold by electrolysis of KAuCl4 using a constant…

A:

Q: Molten SCCI3 can be electrolyzed to form metallic Sc. For what duration should an electrolysis be…

A: We have to calculate the time needed for deposit of the metal.

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: Given data are as follows: Cell potential =- 0.201 V Temperature = 298 K Pressure = 1 atm.

Q: An unstirred solution of 2.00 M NaCl was electrolyzed for a period of 28.9 min and then titrated…

A: Concentration of NaCl = 2M Time duration of electrolysis = 28.9min Concentration of HCl = 0.314M…

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.